Enthalpy for the reaction ${\mathrm{Ag}}^{+}\left(\mathrm{aq}\right)+{\mathrm{Br}}^{-}\left(\mathrm{aq}\right)\to \mathrm{AgBr}\left(\mathrm{s}\right)$ is $-84.54 \mathrm{kJ}$. Magnitude of enthalpy of formation of ${\mathrm{Ag}}^{+}\left(\mathrm{aq}\right)$ and ${\mathrm{Br}}^{-}\left(\mathrm{aq}\right)$ are in the ratio $8 : 9$. Formation of ${\mathrm{Ag}}^{+}\left(\mathrm{aq}\right)$ is an endothermic process whereas formation of ${\mathrm{Br}}^{-}$ is an exothermic process. Enthalpy of formation of $\mathrm{AgBr}$ is $-99.54 \mathrm{kJ}/\mathrm{mol}$. Calculate the enthalpy of formation of ${\mathrm{Ag}}^{+}\left(\mathrm{aq}\right)$ in $\mathrm{kJ}/\mathrm{mol}$.

Given are the following standard free energies of formation at $298 \mathrm{K}$.

$\begin{array}{lllll}& \mathrm{CO}\left(\mathrm{g}\right)& {\mathrm{CO}}_2\left(\mathrm{g}\right)& {\mathrm{H}}_2\mathrm{O}\left(\mathrm{g}\right)& {\mathrm{H}}_2\mathrm{O}\left(\mathrm{l}\right)\\ \frac{{\mathrm{\Delta }}_{\mathrm{f}}\mathrm{G}°}{{\mathrm{kJmole}}^{-1}}& -137.17& -394.36& -228.57& -237.13\end{array}$

(a) Find ${\mathrm{\Delta }}_{\mathrm{r}}\mathrm{G}°$ and the standard equilibrium constant ${\mathrm{K}}_{\mathrm{p}}^0$ at $298 \mathrm{K}$ for the reaction
$\mathrm{CO}\left(\mathrm{g}\right)+{\mathrm{H}}_2\mathrm{O}\left(\mathrm{g}\right)\rightleftharpoons {\mathrm{CO}}_2\left(\mathrm{g}\right)+{\mathrm{H}}_2\left(\mathrm{g}\right)$

(b) If $\mathrm{CO},{\mathrm{CO}}_2$ and ${\mathrm{H}}_2$ are mixed so that the partial pressure of each is $101.325 \mathrm{kPa}$ and the mixture is brought into contact with excess of liquid water, what will be the partial pressure of each gas when equilibrium is attained at $298 \mathrm{K}$. The volume available to the gases is constant.